Chemistry 102(01) Spring 2002 n Instructor: Dr. Upali Siriwardane n e-mail:[email protected] n Office: CTH 311 Phone 257-4941 n Office Hours: n 8:00-9:00.
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Chemistry 102(01) Spring 2002 Instructor: Dr. Upali Siriwardane e-mail:[email protected] Office: CTH 311 Phone 257-4941 Office Hours: 8:00-9:00 & 11:00-12:00 a.m., M, W,
8:00-10:00 a.m., Tu,Th, F
March 27, 2002 (Test 1): Chapter 12 &13. April 26, 2002(Test 2): Chapter 14 & 15. May 15, 2002 (Test 3): Chapter 15 & 17. May 16, 2002 (Comprehensive Test): Chapters 12,13,14,15,17
Chapter 12. Physical Properties of Solutions
solutions Solubility gases :Henry's Law. Concentration units. Energy changes that occur in the solution
process Solubilities of substances in various solvents Colligative properties. Colligative properties of electrolyte solutions. Colloid, true solution and suspension.
Identify Polar and Non-polar groups in Covalent Molecules
Acetic acidHC2H3O2
CH3COOH
HexanolC6H13OH
HexaneC6H14
Propanoic acidC2H5COOH
Like Dissolves Like
Solution Process of Ionic Compounds
Temperature and solubility
0
100
200
300
0 20 40 60 80 100
SO2
KClglycineNaBrKNO3
sucrose
Solu
bili
ty(g
/100
ml w
ate
r)
Temperature (oC)
Pressure and solubility of gases Increasing the pressure of a gas above a
liquid increases the concentration of the gas.
This shifts the equilibrium, driving more gas into the liquid.
Henry's law At constant temperature, the solubility of a
gas is directly proportional to the pressure of the gas above the solution.
S = kH p p= partial pressure of gas above the
solution in atm. S= concentration of gas in the solution
in mol/L. kH= Henry's constant which is
characteristic of the gas and the solvent. S1/S2 =p1/p2
Electrolytes
Solutes which dissolves in water to form conducting solution- Electrolytes
Solutes which dissolves in water to from non-conducting solution-Non- Electrolytes
Solutes which dissolves in water to from weakly conducting solution -Weak- Electrolytes
Concentration Units
a) Molarity (M) b) Normality (N) c) Molality (m) d) Mole fraction (a) e) Mass percent (% weight) f) Volume percent (% volume) g) "Proof" h) ppm and ppb
Molarity(M)
moles of solute Molarity (M) = ------------------------ Liters of solution
Calculate the normality of the solution, which is prepared by dissolving 25 g of H2SO4 in water to a final volume of 2L.M.W. (H2SO4) = 98.08 g/mole
Molality (m)
moles of solute Molality (m) = ------------------------ kg of solvent
Calculate the molality of C2H5OH in water solution which is prepared by mixing 75.0 mL of C2H5OH and 125 g of H2O at 20oC. The density of C2H5OH is 0.789 g/mL.
Mole fraction (a)
moles of solute (substance) a = ------------------------------------- moles of solute + solvent
Calculate the mole fraction of benzene in a benzene(C6H6)-chloroform(CHCl3) solution which contains 60 g of benzene and 30 g of chloroform.M.W. = 78.12 (C6H6) M.W. = 119.37 (CHCl3)
When 100. mL of 0.125 M HCl is diluted to 250. mL, the resulting MOLARITY of the HCl solution is: a) 0.625 M b) 0.250 M c) 0.0500 M d) 0.0250 M e) none of these
Mass (w/w) % or Weight %
Mass of solute Mass (w/w) % = ---------------------- x 100 Mass of solution
What is the mole fraction of ethanol, C2H5OH, in a methanol solution that is 40.%(w/w) ethanol, C2H5OH, by mass?
a. 0.40 b. 0.46 c. 0.21 d. 0.54
Calculate the molarity of a solution of water/alcohol containing 35% C2H5OH by weight. The density of this solution is 1.10 g/mL.
Volume (v/v) % or Volume %
Volume of solute Volume (v/v) % =----------------------x 100 Volume of solution
Proof = Volume % x 2
A solution of hydrogen peroxide is 30.0% H2O2 by mass and has a density of 1.11 g/cm3. The MOLARITY of the solution is: a) 7.94 M b) 8.82 M c) 9.79 M d) 0.980 e) none of these
M.W. = 34.02 (H2O2)
ppm & ppb (w/w or v/v)
Mass (volume) of solute ppm = -------------------------------- x 106 Mass (volume) of solution Mass (volume) of solute ppb = -------------------------------- x 109
The vapor pressure above a glucose-water solution at 25oC is 23.8 torr. What is the mole fraction of glucose (non-dissociating solute) in the solution. The vapor pressure of water at 25oC is 30.5 torr.
At a given temperature the vapor pressures of pure liquid benzene and toluene are 745 torr and 290 torr,respectively. A solution prepared by mixing benzene and toluene obeys Raoult's law. At this temperature the vapor pressure over a solution in which the mole fraction of benzene is equal to 0.340 is
Benzene and toluene form an ideal solution. At 298K, what is the mole fraction of benzene in the liquid that is in equilibrium with a vapor that has equal partial pressures of benzene and toluene? At 298K, the vapor pressures of pure benzene and pure toluene are 95 and 28 torr, respectively. a) 0.50 b) 0.77 c) 0.23 d) 0.30
Boiling Point Elevation (T)
Tb = Kb msolute
Kb = molal boiling point elevation constant
molal means concentration is given in molality(m).
msolute= concentration of solute expressed as molality(m).
What is the boiling point of a 0.500 m aqueous solution of glucose? (Kb for H2O is 0.512 oC/m)
Tb = Kb msolute
Freezing Point Depression (T) Tf = Kf msolute
– Kf = molal Freezing Point Depression
constant
– molal means concentration is given in molality(m).
– msolute= concentration of solute expressed as molality(m).
What is the freezing point of a 0.500 m aqueous solution of glucose? (Kf for H2O is 1.86 oC/m)
Tf = Kf msolute
A 2.25g sample of a compound is dissolved in 125 g of benzene. The freezing point of the solution is 1.02oC. What is the molecular weight of the compound? Kf for benzene = 5.12 oC/m, freezing point = 5.5oC.
Osmotic Pressure
Process of solvent moving through a
semi-permeable membrane is called
Osmosis
The pressure created by moving solvent
is called
Osmotic Pressure
Osmotic Pressure (
= MRT = Osmotic pressure of the solution M= Molarity of the solute in the solution R = Ideal gas constant T= Temperature of the solution in Kelvin
Calculate the osmotic pressure in atm at 20oC of an aqueous solution containing 5.0 g of sucrose (C12H22O11), in 100.0 mL solution.M.W.(C12H22O11)= 342.34
= MRT R = 0.0821 L-atm/mol K = 62.4 L-torr/mol K
Calculation
Ionic vs. covalent substances
Ionic substances have a greater effect per mole than covalent.
1 mol/kg of water for glucose = 1 molal
1 mol/kg of water for NaCl = 2 molal ions
1 mol/kg of water for CaCl2 = 3 molal
ions Effects are based on the number of Effects are based on the number of
particles!particles!
Colligative Properties ofElectrolytes
Number of solute particles in the solution depends on dissociation into ions expressed as Van’t Hoff facotor(i)
Van’t Hoff facotor (i)
moles of particles in solution moles of solutes dissolved
Colligative Properties of Electrolytes Vapor Pressure
Psolution = (1- isolute )Po(solvent) Boiling Point Elevation T = i Kb msolute Freezing Point Depression T = i Kf msolute
Osmotic Pressure = i MRT i =Van’t Hoff factor
Calculate the osmotic pressure in torr of a 0.500 M solution of NaCl in water at 25oC. Assume a 100%dissociation of NaCl.
Calculation
Predict the type of behavior (ideal, negative, positive) based on vapor pressure of the following pairs ofvolatile liquids and explain it in terms of intermolecular attractions: a) Acetone/water(CH3)2CO/H2Ob) Ethanol(C2H5OH)/hexane(C6H14) c) Benzene (C6H6)/toluene CH3C6H5.
Define the Van't Hoff factor (i). Which of the following solutions will show the highest osmotic pressure: a) 0.2 M Na3PO4 b) 0.2 M C6H12O6 (glucose) c) 0.3 M Al2(SO4)3 d) 0.3 M CaCl2 e) 0.3 M NaCl
5.00M.W. = -------- = 128 g/mol 0.0391
a) True solutions (diameter less than 1 x103 pm)b) Colloids (Tyndall effect) (range 1 x103 to 1 x105 pm) c) Suspensions. (greater than 1 x105 pm)